Now, in order to separate the different components of a mixture, it first must be heterogeneous. So, we need them to be in different phases from one another. Now, in this form, each component maintains its individual physical properties. Now, chemical reactions rarely produce a single pure product, so these types of mixtures are common. Now with distillation, we're going to have 2 different apparatuses that we can use for distillation. We're going to say this technique involves the separation of liquids and gases based on a difference in their boiling points. There are many types of distillation methods, but the two most common forms are simple and fractional distillation. So from these two images, the one on the left represents a simple distillation, and the one on the right represents a fractional distillation. Now they have some things in common with one another, but they also have some differences. We're going to say they both have thermometers here, which help to monitor the temperature because we're trying to figure out differences in boiling point. And let's say that both of them have a mixture of 2 compounds, 1 compound A and 1 compound B. And both of them have a heating source. Here this one's using a Bunsen burner, and this one here is using a hot plate. They both serve the same function, to heat up our mixture. And what we're going to say here is that for the simple distillation, and in the fractional distillation, let's say that compound A is methanol. Methanol is an alcohol with a boiling point equal to 67 degrees Celsius. Compound B, let's make it water, which we know its boiling point is 100 degrees Celsius. So both of these sources are going to heat up my mixture. What's going to start happening is they're going to vaporize and become a gas, and they're going to travel up here and up here. In the fractional distillation, we have here what's called a fractional column. We don't have that with simple distillation. In this fractional column, we have little beads. These little beads are supposed to help us to have more surface area for the gas particles to travel to. This also serves another purpose because it helps to lengthen the amount of time it takes for the gas molecules to get through the column. In doing that, some of them are going to recondense back into a liquid. This helps us to increase the cycles of vaporization and condensation. Fractional distillation is a longer process. What happens now is some of the gas particles will travel here, and travel here, and they're going to get to these 2 tubes. Both of them are called Liebig condensers. Basically, they're both connected to hoses. This hose here is cold water that's going into the tube and filling it up here, and this one helps the cold water to exit. You have warm gas traveling through this tube, traveling through this tube, and on either side we have cold water. This is going to help it to condense, and so it's going to drip down as liquid here. With simple distillation, it's faster, and you make a bigger yield of this filtrate here. Unfortunately, it is not as pure. You're going to get, let's say you wanted to isolate ethanol. Ethanol will vaporize sooner because it has a lower boiling point. You're trying to isolate ethanol, but you're going to have a mixture of ethanol and water here. With fractional distillation, the process is longer because it has to travel through the fractional column which has those beads, but you're going to get a much better pure product at the end. Here it's going to be a majority of A. Most of the water is going to recondense back down. Drip into here, get vaporized again, you're going to have more cycles of condensation and vaporization. Now, simple distillation is great if your 2 substances have boiling point differences greater than 25 degrees Celsius. So, in this example where I use methanol and water, their difference in temperature is 33 degrees Celsius. So, simple distillation here will be good. But let's say that we changed compound A from methanol to ethanol. If I change it to that, its boiling point is now 97 degrees Celsius. Those temperatures are too close, so simple distillation will not work. You will need to use fractional distillation. Fractional distillation works better if the boiling point difference between your two liquids is less than 25 degrees Celsius. Here the process is longer, you don't make as much of this filtrate liquid but it's going to be very pure it's going to be more of ethanol or methanol. Now, here if we take a look at this graph, let's say here that we have temperature and we can have it in degrees Celsius or Kelvin, up to you, and it's increasing as we go up. And let's say we're going back to our original methanol, methanol water mix. So here we have mole fraction of methanol, and here we have mole fraction of water. So here let's say we start out with 0 amount of methanol, and here we have just all water. Over time our amount of methanol would increase so 0.20, 0.40, 0.60, 0.80, and then here 100% methanol. And here is 0, 0.20, 0.40, 0.60, and then 0.80. So we're starting out here, and let's say we're starting out with a sample that is, a lot of water initially. As we start to vaporize our mixture, we're trying to get to the point where we have 100% of the filtrate we want, which in this case is ethanol. Each one of these levels represents a vaporization that occurred, Vaporization 123. Because I told you through the glass beads that are in the fractional column, the gases travel, it takes so long that some of it reconnects back into water at the bottom, where it's vaporized again and go through the whole process. We're going to have more instances of vaporization and condensation which causes more cycles of vaporization to happen, with the hope of when you get to your filtrate at the end it's going to be a 100% methanol and 0% of water. And what you have back in the original container that's still on the hotplate is just water. So this is what this is showing us, it's showing us a vaporization-condensation cycle that's occurring within fractional distillation. So just remember, if you're trying to make it quick and try to get the 2 samples separated and the temperatures are greater than 25 degrees Celsius in terms of boiling point, you can go with simple distillation. But if you want a pure filtrate at the end, fractional distillation is the better option.
BONUS: Lab Techniques and Procedures
Distillation & Floatation
BONUS: Lab Techniques and Procedures
Distillation & Floatation - Online Tutor, Practice Problems & Exam Prep
Distillation and Floatation represent procedures that can be used to separate components of a mixture.
Mixture Separation
Distillation can be used to separate liquids or gases based on their different boiling points, while floatation can be used to separate solids based on their different densities.
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Distillation and Floatation
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